CHEMISTRY THE CENTRAL SCIENCE 14TH EDI
14th Edition
ISBN: 9780134863016
Author: Brown
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 2, Problem 11E
A 1.0-g sample of carbon dioxide (002) is fully decomposed into its elements, yielding 0.273 g
of carbon and 0.727 g of oxygen,
a. What is the ratio of the mass of O to C?
b. If a sample of a different compound decomposes into 0.429 g of carbon and 0.571 g of
oxygen, what is its ratio of the mass of O to C?
c. According to Dalton's atomic theory, what is the empirical formula of the second compound?
Expert Solution & Answer
Trending nowThis is a popular solution!
Chapter 2 Solutions
CHEMISTRY THE CENTRAL SCIENCE 14TH EDI
Ch. 2.3 - Which of the following factors determines the size...Ch. 2.3 - Practice Exercise 2 The diameter of a cartoon atom...Ch. 2.3 - Practice Exercise 1 Which of these atoms has the...Ch. 2.3 - Practice Exercise 2
How many protons, neutrons,...Ch. 2.3 - Prob. 2.3.1PECh. 2.3 - Practice Exercise 2
Give the complete chemical...Ch. 2.4 - Practice Exercise 1 There are two stable isotopes...Ch. 2.4 - Practice Exercise 2
Three isotopes of silicon...Ch. 2.5 - Practice Exercise 1 A biochemist who is studying...Ch. 2.5 - Practice Exercise 2 Locate Na (sodium) and Br...
Ch. 2.6 - Practice Exercise 1 Tetra carbon dioxide is an...Ch. 2.6 - Practice Exercise 2 Give the empirical formula for...Ch. 2.7 - Practice Exercise 1 In which of the following...Ch. 2.7 - Practice Exercise 2 How many protons, neutrons,...Ch. 2.7 - Practice Exercise 1
Although it is helpful to...Ch. 2.7 - Prob. 2.8.2PECh. 2.7 - Prob. 2.9.1PECh. 2.7 - Prob. 2.9.2PECh. 2.7 - Prob. 2.10.1PECh. 2.7 - Practice Exercise 2
Write the empirical formula...Ch. 2.8 - Practice Exercise 1 Which of the follow-mg ox...Ch. 2.8 - Prob. 2.11.2PECh. 2.8 - Prob. 2.12.1PECh. 2.8 - Prob. 2.12.2PECh. 2.8 - Prob. 2.13.1PECh. 2.8 - Prob. 2.13.2PECh. 2.8 - Prob. 2.14.1PECh. 2.8 - Practice Exercise 2
Give the chemical fomi uias...Ch. 2.9 - Prob. 2.15.1PECh. 2.9 - Prob. 2.15.2PECh. 2 - Prob. 1ECh. 2 - The followmg diagram is a representation of 20...Ch. 2 - 2 3 Four of the boxes in the following periodic...Ch. 2 -
24 Does the following drawing represent a neutral...Ch. 2 - 2.5 Which of the following diagrams most likely...Ch. 2 - Write the chemical formula for the following...Ch. 2 - Prob. 7ECh. 2 - Prob. 8ECh. 2 - 2.9 Are these two compounds isomers? Explain....Ch. 2 - 2.10 In the Millikan oil-drop experiment (see...Ch. 2 - A 1.0-g sample of carbon dioxide (002) is fully...Ch. 2 - Hydrogen sulfide is composed of two elements:...Ch. 2 - A chemist finds that 30.82 g of nitrogen will...Ch. 2 - 2 . 14 In a series at exper'ments. a chemist...Ch. 2 - 215 Which of the three subatomic particles was...Ch. 2 - 2.16 An unknown particle is caused to move between...Ch. 2 - 2.17 What fraction of α particle in Rutherford’s...Ch. 2 - it 18 Millikan determined the charge on the...Ch. 2 - The radius of an atom of gold (Au) is about 1.35 Å...Ch. 2 - 220 An atom of rhodium (Rh) has a diameter of...Ch. 2 - 2.21 Answer the following questions without...Ch. 2 - Determine whether each of the following statements...Ch. 2 - Consider an atom of "B. a. How many protons,...Ch. 2 - Consider an atom of 63Cu. a. How many protons,...Ch. 2 - 2.25
3. Define atomic number and mass number
b....Ch. 2 -
2 26
Which two of the following are isotopes of...Ch. 2 - How many ptotons, neutrons, and electrons are in...Ch. 2 - 2-28 Each of the following isotopes is used in...Ch. 2 - Prob. 29ECh. 2 - Fill in the gaps in the following table, assuming...Ch. 2 - Write the correct symbol, with both superscript...Ch. 2 - One way in which Earth's evolution as a planet can...Ch. 2 - 2.33
a. What isotope is used as the standard in...Ch. 2 - 2.34
a. What is the mass in amu of a carbon-12...Ch. 2 - Only two isotopes of copper occur naturally:63Cu...Ch. 2 - 2.36 Rubidium has two naturally occurring...Ch. 2 - a. Thomson’s cathode-ray tube (Figure 2.49) and...Ch. 2 -
2.38 Consider the mass spectrometer shown in...Ch. 2 - Naturally occurring magnesium has the following...Ch. 2 - Mass spectrometry is more often applied to...Ch. 2 - 2-41 For each of the following elements, write its...Ch. 2 - Locate each of the following elements in the...Ch. 2 - 2-43 For each of the following elements, write its...Ch. 2 - 2.44 The elements of group 4A show an interesting...Ch. 2 - 2.45 The structural formulas of the compounds...Ch. 2 - 2.46 Ball-and-stick representations of benzene, a...Ch. 2 - 2447 What are the molecular and empirical formulas...Ch. 2 -
2.48 Two substances have the same molecular and...Ch. 2 - 2.49 Write the empirical formula corresponding to...Ch. 2 - Determine the molecular and empirical formulas of...Ch. 2 - 251 How many hydrogen atoms are un each of the...Ch. 2 - Prob. 52ECh. 2 - 253 Write the molecular and structural formulas...Ch. 2 - 2-54 Write the molecular and structural formulas...Ch. 2 - Fill in the gaps in the following table’Ch. 2 - 2.56 Fill in the gaps in the following...Ch. 2 - Each of the following elements is capable of...Ch. 2 - Using the periodic table, predict the charges of...Ch. 2 - 2.59 Using the periodic table to guide you,...Ch. 2 - 2-60 The most common charge associated with...Ch. 2 - 2.61 Predict the chemical formula for the ionic...Ch. 2 - Predict the chemical formulas of the compounds...Ch. 2 - Prob. 63ECh. 2 - Prob. 64ECh. 2 - Predict whether each of the following compounds is...Ch. 2 - 2.66 Which of the following are ionic, and which...Ch. 2 - Prob. 67ECh. 2 - Prob. 68ECh. 2 -
2.69 Give the names and charges of the cation and...Ch. 2 - Give the names and charges of the cation and anion...Ch. 2 -
2.71 Name the following ionic compounds:
a....Ch. 2 - Prob. 72ECh. 2 -
2.73 Write the chemical formulas for the...Ch. 2 -
Give the chemical formula for each of the...Ch. 2 -
2.75 Give the name or chemical formula, as...Ch. 2 - Prob. 76ECh. 2 -
2.T Give the name or Chemical formula, as...Ch. 2 - The oxides of nitrogen are very important...Ch. 2 - Prob. 79ECh. 2 - Assume that you encounter the following sentences...Ch. 2 - a. What is a hydrocarbon? b. Pentane is the alkane...Ch. 2 - 2.82
a. What is meant by the term isomer?
b. Among...Ch. 2 -
2.83
What is a functional group?
What functional...Ch. 2 -
2.84 Consider the following organic substances:...Ch. 2 -
2.85 Chloropropane is derived from propane by...Ch. 2 -
2.86 Draw the structural formulas for three...Ch. 2 - Suppose a scientist repeats the Millikan oil-drop...Ch. 2 -
2.88 The natural abundance of 3He is...Ch. 2 - A cube of gold that is 1.00 cm on a side has a...Ch. 2 -
2.90 The diameter of a rubidium atom is 4.95 A....Ch. 2 -
2.91
Assuming the dimensions of the nucleus and...Ch. 2 -
2.92 Identify the element reoresented by the each...Ch. 2 -
2.93 The nucleus of 6Li is a powerful absorber of...Ch. 2 - The element oxygen has three naturally occurring...Ch. 2 - The element lead (Pb) consists of four naturally...Ch. 2 -
2.96 Gallium (Ga) consists of two naturally...Ch. 2 - Using a suitable reference such as the CRC...Ch. 2 - There are two different isotopes of bromine atoms....Ch. 2 -
2.99 It is common in mass spectrometry to assume...Ch. 2 - From the following list of elements—Ar, H, Ga, Al,...Ch. 2 -
2.101 The first atoms of seaborgium (Sg) were...Ch. 2 -
2.102 The explosion of an atomic bomb releases...Ch. 2 -
2.103. A U.S. 1-cent coin (a penny) has a...Ch. 2 -
2.104 The U.S. Mint produces a dollar coin called...Ch. 2 -
2.105 From the molecular structures shown here,...Ch. 2 -
2.106 Name each of the following oxides. Assuming...Ch. 2 - Prob. 107AECh. 2 -
2.108 Cyclopropane is an interesting hydrocarbon....Ch. 2 - Prob. 109AECh. 2 - Prob. 110AECh. 2 - Give the chemical names of each of the following...Ch. 2 -
2.112 Many familiar substances have common,...Ch. 2 -
2.113 Because many ions and compounds have very...Ch. 2 -
2.114 In what part of the atom does the strong...
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- There are 1.699 1022 atoms in 1.000 g of chlorine. Assume that chlorine atoms are spheres of radius 0.99 and that they are lined up side by side in a 0.5-g sample. How many miles in length is the line of chlorine atoms in the sample?arrow_forwardCopper atoms. (a) What is the average mass of one copper atom? (b) Students in a college computer science class once sued the college because they were asked to calculate the cost of one atom and could not do it. But you are in a chemistry course, and you can do this. (See E. Felsenthal, Wall Street Journal, May 9, 1995.) If the cost of 2.0-mm diameter copper wire (99.9995% pure] is currently 41.70 for 7.0 g, what is the cost of one copper atom?arrow_forwardThe element silver (Ag) has two naturally occurring isotopes: 109 Ag and 107Ag with a mass of 106.905 u. Silver consists of 51.82% 107Ag and has an average atomic mass of 107.868 u. Calculate the mass of 109Ag.arrow_forward
- A sample of metallic element X, weighing 4.315 g, combines with 0.4810 L of Cl2 gas (at normal pressure and 20.0C) to form the metal chloride with the formula XCl. If the density of Cl2 gas under these conditions is 2.948 g/L, what is the mass of the chlorine? The atomic weight of chlorine is 35.45 amu. What is the atomic weight of X? What is the identity of X?arrow_forwardThe early alchemists used to do an experiment in which water was boiled for several days in a sealed glass container. Eventually, some solid residue would appear in the bottom of the flask, which was interpreted to mean that some of the water in the flask had been converted into earth. When Lavoisier repeated this experiment, he found that the water weighed the same before and after heating and the mass of the flask plus the solid residue equaled the original mass of the flask. Were the alchemists correct? Explain what happened. (This experiment is described in the article by A. F. Scott in Scientific American, January 1984.)arrow_forwardWhen a sample of phosphorus burns in air, the compound P4O10 forms. One experiment showed that 0.744 g of phosphorus formed 1.704 g of P4O10. Use this information to determine the ratio of the atomic weights of phosphorus and oxygen (mass P/mass O). If the atomic weight of oxygen is assumed to be 16.000, calculate the atomic weight of phosphorus.arrow_forward
- Constant Composition of Compounds Two samples of sugar are decomposed into their constituent elements. One sample of sugar produces 18.0 g carbon, 3.0 g hydrogen, and 24.0 g oxygen; the other sample produces 24.0 g carbon, 4.0 g hydrogen, and 32.0 g oxygen. Find the ratio of carbon to hydrogen and the ratio of oxygen to hydrogen for each of the samples, and show they are consistent with the law of constant composition.arrow_forward2.92 A candy manufacturer makes chocolate-covered cherries. Although all of the products look roughly the same, 3% of them are missing the cherry. The mass of the candy with a cherry is 18.5 g; those missing the cherry weigh only 6.4 g. (a) How would you compute the average mass of a box of 100 of these chocolate covered cherries from this manufacturer? (b) I low is this question analogous to the determination of atomic weights?arrow_forwardThere are 2.619 1022 atoms in 1.000 g of sodium. Assume that sodium atoms are spheres of radius 1.86 and that they are lined up side by side. How many miles in length is the line of sodium atoms?arrow_forward
- Indium oxide contains 4.784 g of indium for every 1.000 g of oxygen. In 1869, when Mendeleev first presented his version of the periodic table, he proposed the formula In2O3 for indium oxide. Before that time it was thought that the formula was InO. What values for the atomic mass of indium are obtained using these two formulas? Assume that oxygen has an atomic mass of 16.00.arrow_forwardTwo elements, R and Q, combine to form two binary compounds. In the first compound, 14.0 g of R combines with 3.00 g of Q. In the second compound, 7.00 g of R combines with 4.50 g of Q. Show that these data are in accord with the law of multiple proportions. If the formula of the second compound is RQ, what is the formula of the first compound?arrow_forwardEach of the following statements is true, but Dalton might have had trouble explaining some of them with his atomic theory. Give explanations for the following statements. a. The space-filling models for ethyl alcohol and dimethyl ether are shown below. These two compounds have die same composition by mass (52% carbon, 13% hydrogen, and 35% oxygen), yet the two have different melting points, boiling points, and solubilities in water. b. Burning wood leaves an ash that is only a small fraction of the mass of the original wood. c. Atoms can be broken down into smaller particles. d. One sample of lithium hydride is 87.4% lithium by mass, while another sample of lithium hydride Ls 74.9% lithium by mass. However, the two samples have the same chemical properties.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Atomic Number, Atomic Mass, and the Atomic Structure | How to Pass ChemistryThe Nucleus: Crash Course Chemistry #1; Author: Crash Course;https://www.youtube.com/watch?v=FSyAehMdpyI;License: Standard YouTube License, CC-BY